text: Each reaction rate coefficient  has a temperature dependency, which is usually given by the Arrhenius equation:
  where 
  * is the activation energy; 
  * is the gas constant;
  * is the exponential function.
  Since at temperature  the molecules have energies given by a Boltzmann distribution, one can expect the number of collisions with energy greater than  to be proportional to  The coefficient, , is the pre-exponential factor or frequency factor.
  The values for  and  are dependent on the reaction. There are also more complex equations possible, which describe the temperature dependence of other rate constants that do not follow this pattern.
  Temperature is a measure of the average kinetic energy of the reactants. As temperature increases, the kinetic energy of the reactants increases. That is, the particles move faster. With the reactants moving faster this allows more collisions to take place at a greater speed, so the chance of reactants forming into products increases, which in turn results in the rate of reaction increasing. A rise of ten degrees Celsius results in approximately twice the reaction rate.
  The minimum kinetic energy required for a reaction to occur is called the activation energy and is denoted by  or . The transition state or activated complex shown on the diagram is the energy barrier that must be overcome when changing reactants into products. The molecules with an energy greater than this barrier have enough energy to react.
  For a successful collision to take place, the collision geometry must be right, meaning the reactant molecules must face the right way so the activated complex can be formed.
  A chemical reaction takes place only when the reacting particles collide. However, not all collisions are effective in causing the reaction. Products are formed only when the colliding particles possess a certain minimum energy called threshold energy. As a rule of thumb, reaction rates for many reactions double for every ten degrees Celsius increase in temperature. For a given reaction, the ratio of its rate constant at a higher temperature to its rate constant at a lower temperature is known as its temperature coefficient, ().  Q is commonly used as the ratio of rate constants that are ten degrees Celsius apart.